Discussion
A gaseous fuel mixture comprising 3 moles of methane and 2 moles of ammonia is combusted in X moles of pure oxygen in stoichiometric amount. Assuming complete combustion, with only CO2, H2O and N2 in the product gases, the value of X is ___.
3 CH4 + 2 NH3 + X O2 → Products (CO2, H2O, N2)
Answer: A
The value of X is 7.5.
Balance each fuel separately for complete combustion:
\[ \begin{aligned} CH_{4} + 2O_{2} &\to CO_{2} + 2H_{2}O \\ 2NH_{3} + 1.5O_{2} &\to N_{2} + 3H_{2}O \end{aligned} \]
Three moles of methane need 3 × 2 = 6 moles of O2, and two moles of ammonia need 1.5 moles, so X = 7.5. Check by atoms: 3 C, 18 H and 4 N give 3 CO2, 9 H2O and 2 N2, containing 6 + 9 = 15 O atoms, that is 7.5 O2. None of the other values balances the oxygen atoms.
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